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  • Is aluminium a metal or metalloid? - Chemistry Stack Exchange
    Aluminium is usually considered to be a metal, as described in the Wikipedia article Metalloids: Aluminium: Aluminium is ordinarily classified as a metal It is lustrous, malleable and ductile, and has high electrical and thermal conductivity Like most metals it has a close-packed crystalline structure, and forms a cation in aqueous solution
  • Why cant Al3+ be reduced to solid, pure aluminum?
    So the aluminium oxide is reduced via the Hall–Héroult process The alumina itself is produced from mined bauxite via the Bayer process So the gist is that industry spends many many millions of dollars converting bauxite too aluminium metal No doubt they do it the cheapest way possible
  • Why is Aluminium oxide amphoteric? - Chemistry Stack Exchange
    Metal hydroxides are basic in water Non-metal oxides are acids in water The limit between metals and non-metals is a sort of staircase going through the periodic table from the middle of the first line to the lower corner at the right-hand side Aluminium touches this staircase
  • Chemical Reaction of aluminum foil in CuCl2 solution
    Now, for the experiment discussed with Al CuCl2, I suspect elemental copper metal, especially freshly precipitated, will similarly react forming a coating of cuprous oxide per the normally slow observed oxidation of iron and copper metal in an acidic air CO2 mix per the so called metal auto-oxidation reaction (Reaction R24 above):
  • metal - Does the protective layer of Aluminum oxide form on the surface . . .
    Aluminum is an ideal element for usage in airports Unlike Iron, when oxygenating, there is a protective layer formed that does not allow the rest of the Al metal to oxygenate Does the protective layer $\ce{Al2O3}$ form on the surface of aluminum alloys (such as Al-Zr) as well as when it happens to Aluminum in its pure state?
  • electrochemistry - Bubble formation when aluminium reacts with copper . . .
    If the $\ce{CuSO4}$ solution is acidic enough, the $\ce{Al(OH)3}$ rapidly dissolves, exposing a fresh aluminium surface, ready for further reaction On the other hand, the redox reaction of $\ce{Fe(s)}$ and water is not favorable enough for hydrogen evolution to occur, which explains the lack of bubbles you observed
  • Why do only some metals make protective oxide layers?
    Like a clay layer, the hydroxide ions fuzz out of each layer of close-packed magnesium ions, and the metal surface could be like a half-layer of $\ce{Mg(OH)2}$, with $\ce{OH-}$ ions sticking out and bonding to separate layers of $\ce{Mg(OH)2}$, or perhaps the metal itself just hold onto a layer of $\ce{Mg(OH)2}$ - or maybe a little of both This adherence is necessary to stifle corrosion
  • inorganic chemistry - How does Aluminum react with nitric acid at . . .
    The qualifications for dissolution is interesting as it amounts basically to a galvanic cell anodic dissolution (think 'Bleach Battery' variation with HNO3 in place of HOCl and a copper metal electrode, the latter created from Aluminum displacing Cu(II) ions forming a Cu cathode on the Al surface)
  • What causes passivity of specific metals in conc. nitric acid?
    Aluminium This link states that: Aluminium metal dissolves readily in dilute sulphuric acid to form solutions containing the hydrated Al(III) ion together with hydrogen gas, $\ce{H2}$ The corresponding reactions with dilute hydrochloric acid also give the hydrated Al(III) ion
  • inorganic chemistry - Anodisation of aluminium in sulfuric acid . . .
    As an experiment for electrolysis and to show how a metal can be protected of corrosion, I am trying to anodize an aluminium plate, using sulfuric acid as electrolyte I know the aluminium plate is the cathode and, thus, connected to the positive terminal of the generator, while for the cathode I am using aluminium foil





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